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2 years ago

Is the process of bananas ripening a chemical change or a physical change? explain?

1 answer:

7 0

Bananas ripening is a chemical change. First, there is a change in color of peel from green to yellow then to brown. Second, there is a change in taste. You will notice a change in taste as the bananas ripen. They become sweeter and sweeter as they begin to ripen.

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Which prey is common to all owls?

IrinaK [193]

Answer:

Mice

Explanation:

Small, rodent-like mammals, such as voles and mice, are the primary prey for many owl species. An owl's diet may also include frogs, lizards, snakes, fish, mice, rabbits, birds, squirrels, and other creatures. Occasionally, Great Horned Owls might even find skunks tasty enough to eat.

Please mark brainliest! I only need one more to rank up! Thank you and have a blessed day/night :D

8 0

2 years ago

Read 2 more answers

Which pair of aqueous solutions can create a buffer solution if present in the appropriate concentrations?.

Julli [10]

HF and NaF - If the right concentrations of aqueous solutions are present, they can produce a buffer solution.

<h3>What are buffer solutions and how do they differ?</h3>

The two main categories of buffers are acidic buffer solutions and alkaline buffer solutions.
Acidic buffers are solutions that contain a weak acid and one of its salts and have a pH below 7.
For instance, a buffer solution with a pH of roughly 4.75 is made of acetic acid and sodium acetate.

<h3>Describe buffer solution via an example.</h3>

When a weak acid or a weak base is applied in modest amounts, buffer solutions withstand the pH shift.
A buffer made of a weak acid and its salt is an example.
It is a solution of acetic acid and sodium acetate CH3COOH + CH3COONa.

learn more about buffer solutions here

<u>brainly.com/question/8676275</u>

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8 0

11 months ago

Adding a catalyst to a system at equilibrium lowers the activation energy required by a system, which system, which shifts the e

GarryVolchara [31]

Answer: False

Explanation: Took the test

8 0

2 years ago

Read 2 more answers

Given 3.4 grams of x compound with a molar mass of 85 g and 4.2 grams of y compound with a molar mass of 48 g How much of compou

Ulleksa [173]

Answer:

$4.36~g~XY$

Explanation:

In this case, we can start with the reaction:

$2X + Y_2~->~2XY$

If we check the reaction, we will have 2 X and Y atoms on both sides. So, <u>the reaction is balanced</u>. Now, the problem give to us two amounts of reagents. Therefore, we have to find the <u>limiting reagent</u>. The first step then is to find the moles of each compound using the <u>molar mass</u>:

$3.4~g~X\frac{1~mol~X}{85~g~X}=0.04~mol~X$

$4.2~g~Y_2\frac{1~mol~Y_2}{48~g~Y_2}=0.0875~mol~Y_2$

Now, we can <u>divide by the coefficient</u> of each compound (given by the balanced reaction):

$\frac{0.04~mol~X}{1}=~0.04$

$\frac{0.0875~mol~Y_2}{2}=0.04375$

The smallest value is for "X", therefore this is our <u>limiting reagent</u>. Now, if we use the <u>molar ratio</u> between "X" and "XY" we can calculate the moles of XY, so:

$0.04~mol~X\frac{2~mol~XY}{2~mol~X}=0.04~mol~XY$

Finally, with the molar mass of "XY" we can calculate the grams. Now, we know that 1 mol X = 85 g X and 1 mol $Y_2$ = 48 g $Y_2$ (therefore 1 mol Y = 24 g Y). With this in mind the <u>molar mass of XY</u> would be 85+24 = 109 g/mol. With this in mind:

$0.04~mol~XY\frac{109~g~XY}{1~mol~XY}=4.36~g~XY$

I hope it helps!

6 0

3 years ago

Suppose there is a gaseous mixture of nitrogen and oxygen. If the total pressure of the mixture is 480 mmHg, and the partial pre

Rudiy27

Answer:

Partial pressure of oxygen = 190 mmHg

Explanation:

From the question;

Mixture contains only nitrogen and oxygen

Total pressure of the mixture = 480 mmHg

Partial pressure of nitrogen = 290 mmHg

Dalton's law states that the pressure of a system is as a result of the sum of the partial pressures of the individual components of the mixture. This means that in this mixture;

Pressure of mixture = Partial Pressure of Nitrogen + Partial Pressure of Oxygen

480 = 290 + Partial pressure of oxygen

Partial pressure of oxygen = 480 - 290

Partial pressure of oxygen = 190 mmHg

3 0

2 years ago